Question

If butane had a volume of 500 mL. at a pressure of 1.5 atm and a temperature of
20 °C, what would the new volume of the gas be at a temperature of 30 °C and a pressure
of 500 Torr

Answer 1

Question:

If butane had a volume of 500 ml. at a pressure of 1.5 atm and a temperature of 20 °C, what would the new volume of the gas be at a temperature of 30 °C and a pressure of 500 Torr?

Solution Given:

Let P be the pressure V be volume and and T be temperature.

Volume of Butane [$V_1$] = 500 ml

Pressure of Butane [$P_1$] = 1.5 atm

Temperature [$T_1$] =20°C=20+273=293K

New Volume of Butane [$V_2$] = ?

New Pressure of Butane [$V_2$] =500 Torr=500*0.00131579=0.657895 atm

Note: 1 Torr= 0.00131579 atm

New Temperature of Butane [$V_2$] =30°C=30+273=303K

Now

By using combined gas law equation:

$V_2=V_2*\frac{P_1*T_2}{P_2*T_1}$

$V_2=500*\frac{1.5*303}{0.657895*293}=1178.9 ml$

The new volume of Butane is 1178.9 ml